The ionic strength of a
solution
Solution may refer to:
* Solution (chemistry), a mixture where one substance is dissolved in another
* Solution (equation), in mathematics
** Numerical solution, in numerical analysis, approximate solutions within specified error bounds
* Solutio ...
is a measure of the
concentration
In chemistry, concentration is the abundance of a constituent divided by the total volume of a mixture. Several types of mathematical description can be distinguished: '' mass concentration'', '' molar concentration'', ''number concentration'', ...
of
ions in that solution. Ionic
compounds, when
dissolved in water,
dissociate into ions. The total
electrolyte
An electrolyte is a medium containing ions that is electrically conducting through the movement of those ions, but not conducting electrons. This includes most soluble salts, acids, and bases dissolved in a polar solvent, such as water. Upon ...
concentration in solution will affect important properties such as the
dissociation constant
In chemistry, biochemistry, and pharmacology, a dissociation constant (K_D) is a specific type of equilibrium constant that measures the propensity of a larger object to separate (dissociate) reversibly into smaller components, as when a complex ...
or the
solubility
In chemistry, solubility is the ability of a substance, the solute, to form a solution with another substance, the solvent. Insolubility is the opposite property, the inability of the solute to form such a solution.
The extent of the solubi ...
of different
salts. One of the main characteristics of a solution with dissolved ions is the ionic strength. Ionic strength can be
molar (mol/L solution) or
molal (mol/kg solvent) and to avoid confusion the units should be stated explicitly. The concept of ionic strength was first introduced by
Lewis and
Randall Randall may refer to the following:
Places
United States
*Randall, California, former name of White Hall, California, an unincorporated community
* Randall, Indiana, a former town
*Randall, Iowa, a city
*Randall, Kansas, a city
*Randall, Minnesot ...
in 1921 while describing the
activity coefficient
In thermodynamics, an activity coefficient is a factor used to account for deviation of a mixture of chemical substances from ideal behaviour. In an ideal mixture, the microscopic interactions between each pair of chemical species are the same ...
s of
strong electrolytes.
Quantifying ionic strength
The molar ionic strength, ''I'', of a solution is a function of the
concentration
In chemistry, concentration is the abundance of a constituent divided by the total volume of a mixture. Several types of mathematical description can be distinguished: '' mass concentration'', '' molar concentration'', ''number concentration'', ...
of ''all''
ions present in that
solution
Solution may refer to:
* Solution (chemistry), a mixture where one substance is dissolved in another
* Solution (equation), in mathematics
** Numerical solution, in numerical analysis, approximate solutions within specified error bounds
* Solutio ...
.
:
where one half is because we are including both
cation
An ion () is an atom or molecule with a net electrical charge.
The charge of an electron is considered to be negative by convention and this charge is equal and opposite to the charge of a proton, which is considered to be positive by conven ...
s and
anion
An ion () is an atom or molecule with a net electrical charge.
The charge of an electron is considered to be negative by convention and this charge is equal and opposite to the charge of a proton, which is considered to be positive by conve ...
s, ''c''
i is the
molar concentration of ion i (M, mol/L), ''z''
i is the
charge number of that ion, and the sum is taken over all ions in the solution. For a 1:1
electrolyte
An electrolyte is a medium containing ions that is electrically conducting through the movement of those ions, but not conducting electrons. This includes most soluble salts, acids, and bases dissolved in a polar solvent, such as water. Upon ...
such as
sodium chloride
Sodium chloride , commonly known as salt (although sea salt also contains other chemical salts), is an ionic compound with the chemical formula NaCl, representing a 1:1 ratio of sodium and chloride ions. With molar masses of 22.99 and 35. ...
, where each ion is singly-charged, the ionic strength is equal to the concentration. For the electrolyte
MgSO4, however, each ion is doubly-charged, leading to an ionic strength that is four times higher than an equivalent concentration of sodium chloride:
:
Generally
multivalent ions contribute strongly to the ionic strength.
Calculation example
As a more complex example, the ionic strength of a mixed solution 0.050 M in Na
2SO
4 and 0.020 M in KCl is:
:
Non-ideal solutions
Because in non-
ideal solutions volumes are no longer strictly additive it is often preferable to work with
molality
Molality is a measure of the number of moles of solute in a solution corresponding to 1 kg or 1000 g of solvent. This contrasts with the definition of molarity which is based on a specified volume of solution.
A commonly used unit for molali ...
''b'' (mol/kg of H
2O) rather than molarity ''c'' (mol/L). In that case, molal ionic strength is defined as:
:
in which
:''i'' = ion identification number
:''z'' = charge of ion
:''b'' = molality (mol solute per Kg solvent)
Importance
The ionic strength plays a central role in the
Debye–Hückel theory
The Debye–Hückel theory was proposed by Peter Debye and Erich Hückel as a theoretical explanation for departures from ideality in solutions of electrolytes and plasmas.
It is a linearized Poisson–Boltzmann model, which assumes an extrem ...
that describes the strong deviations from ideality typically encountered in ionic solutions.
It is also important for the theory of
double layer and related
electrokinetic phenomena and
electroacoustic phenomena in
colloids and other
heterogeneous
Homogeneity and heterogeneity are concepts often used in the sciences and statistics relating to the uniformity of a substance or organism. A material or image that is homogeneous is uniform in composition or character (i.e. color, shape, siz ...
systems. That is, the
Debye length, which is the inverse of the Debye parameter (''κ''), is inversely proportional to the square root of the ionic strength. Both molar and molal ionic strength have been used, often without explicit definition. Debye length is characteristic of the double layer thickness. Increasing the concentration or
valence of the
counterion
160px, Polystyrene sulfonate, a cation-exchange resin, is typically supplied with as the counterion.">cation-exchange_resin.html" ;"title="Polystyrene sulfonate, a cation-exchange resin">Polystyrene sulfonate, a cation-exchange resin, is typical ...
s compresses the double layer and increases the
electrical potential gradient
In vector calculus, the gradient of a scalar-valued differentiable function of several variables is the vector field (or vector-valued function) \nabla f whose value at a point p is the "direction and rate of fastest increase". If the gr ...
.
Media of high ionic strength are used in
stability constant determination in order to minimize changes, during a titration, in the activity quotient of solutes at lower concentrations. Natural waters such as
mineral water and
seawater
Seawater, or salt water, is water from a sea or ocean. On average, seawater in the world's oceans has a salinity of about 3.5% (35 g/L, 35 ppt, 600 mM). This means that every kilogram (roughly one liter by volume) of seawater has appro ...
have often a non-negligible ionic strength due to the presence of dissolved salts which significantly affects their properties.
See also
*
Activity (chemistry)
*
Activity coefficient
In thermodynamics, an activity coefficient is a factor used to account for deviation of a mixture of chemical substances from ideal behaviour. In an ideal mixture, the microscopic interactions between each pair of chemical species are the same ...
*
Bromley equation
The Bromley equation was developed in 1973 by Leroy A. Bromley with the objective of calculating activity coefficients for aqueous electrolyte solutions whose concentrations are above the range of validity of the Debye–Hückel equation. This equa ...
*
Davies equation
*
Debye–Hückel equation
*
Debye–Hückel theory
The Debye–Hückel theory was proposed by Peter Debye and Erich Hückel as a theoretical explanation for departures from ideality in solutions of electrolytes and plasmas.
It is a linearized Poisson–Boltzmann model, which assumes an extrem ...
*
Double layer (interfacial)
*
Double layer (electrode)
A double layer (DL, also called an electrical double layer, EDL) is a structure that appears on the surface of an object when it is exposed to a fluid. The object might be a solid particle, a gas bubble, a liquid droplet, or a porous body. The D ...
*
Double layer forces
*
Electrical double layer
A double layer (DL, also called an electrical double layer, EDL) is a structure that appears on the surface of an object when it is exposed to a fluid. The object might be a solid particle, a gas bubble, a liquid droplet, or a porous body. The D ...
*
Gouy-Chapman model
*
Flocculation
Flocculation, in the field of chemistry, is a process by which colloidal particles come out of suspension to sediment under the form of floc or flake, either spontaneously or due to the addition of a clarifying agent. The action differs from ...
*
Peptization (the inverse of flocculation)
*
DLVO theory (from Derjaguin, Landau, Verwey and Overbeek)
*
Interface and colloid science
*
Osmotic coefficient
*
Pitzer equations
*
Poisson–Boltzmann equation
*
Specific ion Interaction Theory
In theoretical chemistry, Specific ion Interaction Theory (SIT theory) is a theory used to estimate single-ion activity coefficients in electrolyte solutions at relatively high concentrations. It does so by taking into consideration ''interaction ...
*
Salting in
*
Salting out
Salting out (also known as salt-induced precipitation, salt fractionation, anti-solvent crystallization, precipitation crystallization, or drowning out) is a purification technique that utilizes the reduced solubility of certain molecules in a s ...
External links
Ionic strengthIonic strength introduction at the EPA web site
References
{{Authority control
Analytical chemistry
Colloidal chemistry
Electrochemical equations
Electrochemical concepts
Equilibrium chemistry
Physical chemistry
Physical quantities